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Question:

In a bimolecular reaction, the steric factor P was experimentally determined to be 4.5. The correct option(s) among the following is (are):
Experimentally determined value of frequency factor is higher than that predicted by Arrhenius equation.
The value of frequency factor predicted by Arrhenius equation is higher than that determined experimentally.
The activation energy of the reaction is unaffected by the value of the steric factor.
Since P=4.5, the reaction will not proceed unless an effective catalyst is used.

SinceP=4.5, the reaction will not proceed unless an effective catalyst is used.

Experimentally determined value of frequency factor is higher than that predicted by Arrhenius equation.

The value of frequency factor predicted by Arrhenius equation is higher than that determined experimentally.

The activation energy of the reaction is unaffected by the value of the steric factor.

Solution:

P=4.5 ⇒ P>1
We know, Kexp/Kcollision = P
Kexp = PAe^(-Ea/RT)
Aexp = PA
⇒ Aexp > A
⇒ experimentally determined value of frequency factor is higher than that predicted by Arrhenius equation.
⇒ option A is correct and B is incorrect.
Kexp = PAe^(-Ea/RT)
Since in this equation Ea is not changed, option C is correct.
Since Kexp > K, there is no need of an effective catalyst to reduce activation energy so that Kexp increases.
⇒ option D is not correct.